Ammonia Production and Yield Calculations

The video tutorial explains the concept of limiting reactants in chemical reactions, using ammonia production as an example. It describes how to determine the limiting reactant and calculate the mass of products formed. The tutorial also covers percent yield and theoretical yield, providing a comprehensive understanding of these concepts in the context of chemical reactions.

What is the term used for the reactant that determines the maximum amount of product formed in a chemical reaction?

• Excess reactant

• Limiting reactant

• Catalyst

• Inert reactant

In the reaction to form ammonia, how many moles of hydrogen gas are required to react with one mole of nitrogen gas?

• One mole

• Two moles

• Three moles

• Four moles

If you start with 8 molecules of hydrogen and 8 molecules of nitrogen, how many molecules of ammonia can be produced?

• Two molecules

• Four molecules

• Six molecules

• Eight molecules

What is the molar mass of nitrogen gas (N2) used in the calculations?

• 44 g/mol

• 32 g/mol

• 28 g/mol

• 14 g/mol

How many grams of ammonia are produced when 155 grams of nitrogen react completely?

• 143 grams

• 155 grams

• 317 grams

• 188 grams

What is the mass of hydrogen left over when 155 grams of nitrogen react with 56 grams of hydrogen?

• 0 grams

• 56 grams

• 33.2 grams

• 22.8 grams

What does the percent yield compare in a chemical reaction?

• Initial mass to final mass

• Limiting reactant to excess reactant

• Reactants to products

• Theoretical yield to actual yield

If the actual yield of ammonia is 143 grams, what is the percent yield given a theoretical yield of 188 grams?

• 90%

• 76%

• 80%

• 85%

Which factor is NOT considered when calculating the percent yield?

• Theoretical yield

• Molar mass of reactants

• Reaction temperature

• Actual yield

What is the theoretical yield of ammonia when 155 grams of nitrogen and 56 grams of hydrogen are reacted?

• 143 grams

• 317 grams

• 188 grams

• 56 grams